(a)
Interpretation:
The oxidation number for atoms in
Concept introduction:
Oxidation number:
The oxidation number of an element is zero. The oxidation number of a monoatomic ion equals its charge.
The oxidation number is zero for the summation of the oxidation numbers complete atoms in a complete formula.
The charge on the ion is equal to the summation of the oxidation numbers of complete atoms in poly atomic ion.
The oxidation state of alkali metal
The oxidation state of hydrogen is
(b)
Interpretation:
The oxidation number for all atoms in
Concept introduction:
Refer to part (a)
(c)
Interpretation:
The oxidation number for all atoms in
Concept introduction:
Refer to part (a)
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry: The Molecular Science
- Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.arrow_forwardIron forms a sulfide with the approximate formula Fe7S8. Assume that the oxidation state of sulfur is 2 and that iron atoms exist in both +2 and +3 oxidation states. What is the ratio of Fe(II) atoms to Fe(III) atoms in this compound?arrow_forwardA 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?arrow_forward
- 4.22 Generally, an excess of O2 is needed for the reaction Sn+O2SnO2 . What is the minimum number of moles of oxygen required to oxidize 7.3 moles of tin?arrow_forwardA 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ion, which was then precipitated with an excess of potassium chromate to give 2.012 g of barium chromate, BaCrO4. What is the formula of the compound?arrow_forwardMagnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?arrow_forward
- Given HFH+(aq)+F(aq)Ka=6.9104HF(aq)+F(aq)H2(aq)K=2.7 calculate K for the reaction 2HF(aq)H+(aq)+HF2(aq)arrow_forwardA 0.709 g sample of H2C2O4·2H2O is dissolved in water and titrated to a phenolphthalein endpoint with 27.98 mL of a sodium hydroxide solution. What is the molarity of the NaOH?arrow_forwardYou are assigned to prepare a 500.0 mL of a2.80 M solution of KI. (a) What would you do first? (b)Describe the necessary steps for the preparation of thissolution in the laboratory.arrow_forward
- Name the products formed in each case when(a) hydrochloric acid reacts with caustic soda.(b) granulated zinc reacts with caustic soda.(c) carbon dioxide is passed into lime water.arrow_forwardPredict the product(s) and write a balanced equation for eachof the following redox reactions:(a) Cesium+ iodine→ (b) Aluminum+ aqueous manganese(II) sulfate→ (c) Sulfur dioxide +oxygen→ (d) Butane and oxygen→ (e) Write a balanced net ionic equation for (b)arrow_forwardWhen a solution of dithionite ions (S2O42–) is added to a solution of chromate ions (CrO42–), the products of the ensuing chemical reaction, which occurs under basic conditions, include soluble sulfite ions and solid chromic hydroxide. This reaction is used to remove Cr(VI) from wastewater generated by factories that make chrome-plated metals. (a) Write the net ionic equation for this reaction. Do not include phases. (b) How many grams of sodium dithionite would be needed to remove the Cr(VI) in 115 L of wastewater that contains 1.43×10-3 M chromate ions?arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning